Year 11 Science - Chemistry Revision 1

In this mix (video), I will cover the basics of atoms, elements and how to combine elements into ionic compounds.

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Year 11 Science - Chemistry Revision 1

Created 2 years ago

Duration 0:18:31
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In this mix (video), I will cover the basics of atoms, elements and how to combine elements into ionic compounds.
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Slide Content
  1. Introduction

    Slide 1 - Introduction

    • As the end of topic test for Year 11 chemistry is coming up, I thought it is a good idea to go through some scientific concepts about chemistry.
    • In this first part of two episodes, I am going to talk about atoms, elements and ions.
    • Welcome to this episodes of daily science, where science is all about invention, imagination and inspiration.
  2. Atoms

    Slide 2 - Atoms

    • Atoms are the basic building block of all matter
    • Cheese Atom
  3. Atomic Structure

    Slide 3 - Atomic Structure

    • Atom is consisted:
    • Electrons
    • Neutrons
    • Protons
    • -
    • +
    • +
    • -
    • Nucleus
    • Electron Shell
    • Electron
    • Neutron
    • Proton
    • Proton
    • Electron
    • Neutron
    • I am positive!
    • I am negative
    • I just don’t care
  4. Electron shells

    Slide 4 - Electron shells

    • -
    • +
    • +
    • -
    • Electron Shell
    • Helium
    • -
    • +
    • +
    • -
    • Electron Shell
    • Lithium
    • +
    • -
    • Shell
    • Number of electron
    • 1 (The most inner shell)
    • 2
    • 2
    • 8
    • 3
    • 8
    • 4
    • 2
  5. Elements

    Slide 5 - Elements

    • Elements are the simplest substances and each element is made up of just one particular type of atom. Each element can be represented by a symbol.
    • Gold (Au) is an element made up of only gold atoms.
    • Carbon (C) is an element made up of only carbon atoms.
  6. Ions

    Slide 6 - Ions

    • Elements are electrically neutral but not necessary stable
    • Contain equal amount of positive and negative charge (protons and electrons)
    • Elements that have lost or gained electrons in chemical reaction are called ions.
    • The number of electrons that are gained and lost are determined by the number of electrons in the outer (valence) shell
    • Elements are more stable if their valence shell is completely full or empty
  7. Slide 7

    • Ions
    • -
    • +
    • +
    • -
    • Lithium
    • +
    • -
    • Shell
    • Number of electron
    • 1 (The most inner shell)
    • 2
    • 2
    • 8
    • 3
    • 8
    • 4
    • 2
    • Li
    • Li+ ion
    • Free Electron
    • -
    • -
    • Chlorine
    • +
    • +
    • +
    • +
    • +
    • +
    • +
    • +
    • +
    • +
    • +
    • -
    • -
    • -
    • -
    • -
    • -
    • -
    • -
    • -
    • -
    • -
    • -
    • -
    • -
    • -
    • Cl
    • Cl- ion
    • Lithium Chloride
    • LiCl
  8. Naming ionic compounds – Three rules

    Slide 8 - Naming ionic compounds – Three rules

    • The name for the positive ion always comes first
    • When there are only two elements in the compound, the name usually ends in –ide. For example: sodium chloride ()
    • A name ending in –ate or –ite means that the compound contains oxygen and another non-metal. For example: copper sulphate (
  9. Ionic compound

    Slide 9 - Ionic compound

    • Example: Sodium and Chlorine
    • +1
    • +2
    • +3
    • -3
    • -2
    • -1
    • NH4+
    • Ammonium
    • Ca2+
    • Calcium
    • Al3+
    • Aluminium
    • O2-
    • Oxide
    • OH-
    • Hydroxide
    • Na+
    • Sodium
    • Mg2+
    • Magnesium
    • Fe3+
    • Iron (III)
    • S2-
    • Sulphide
    • Cl-
    • Chloride
    • K+
    • Potassium
    • Cu2+
    • Copper
    • CO32-
    • Carbonate
    • NO3-
    • Nitrate
    • Ag+
    • Silver
    • Pb2+
    • Lead
    • SO42-
    • Sulphate
    • HCO3-
    • Hydrogen carbonate
    • H+
    • Hydrogen
    • Fe2+
    • Iron (II)
    • Ba2+
    • Barium
    • Zn2+
    • Zinc
  10. Ionic compound

    Slide 10 - Ionic compound

    • Example: Aluminium and Hydroxide
    • +1
    • +2
    • +3
    • -3
    • -2
    • -1
    • NH4+
    • Ammonium
    • Ca2+
    • Calcium
    • Al3+
    • Aluminium
    • O2-
    • Oxide
    • OH-
    • Hydroxide
    • Na+
    • Sodium
    • Mg2+
    • Magnesium
    • Fe3+
    • Iron (III)
    • S2-
    • Sulphide
    • Cl-
    • Chloride
    • K+
    • Potassium
    • Cu2+
    • Copper
    • CO32-
    • Carbonate
    • NO3-
    • Nitrate
    • Ag+
    • Silver
    • Pb2+
    • Lead
    • SO42-
    • Sulphate
    • HCO3-
    • Hydrogen carbonate
    • H+
    • Hydrogen
    • Fe2+
    • Iron (II)
    • Ba2+
    • Barium
    • Zn2+
    • Zinc
  11. Ionic compound

    Slide 11 - Ionic compound

    • Example: Iron (III) and Carbonate
    • +1
    • +2
    • +3
    • -3
    • -2
    • -1
    • NH4+
    • Ammonium
    • Ca2+
    • Calcium
    • Al3+
    • Aluminium
    • O2-
    • Oxide
    • OH-
    • Hydroxide
    • Na+
    • Sodium
    • Mg2+
    • Magnesium
    • Fe3+
    • Iron (III)
    • S2-
    • Sulphide
    • Cl-
    • Chloride
    • K+
    • Potassium
    • Cu2+
    • Copper
    • CO32-
    • Carbonate
    • NO3-
    • Nitrate
    • Ag+
    • Silver
    • Pb2+
    • Lead
    • SO42-
    • Sulphate
    • HCO3-
    • Hydrogen carbonate
    • H+
    • Hydrogen
    • Fe2+
    • Iron (II)
    • Ba2+
    • Barium
    • Zn2+
    • Zinc
  12. Ionic compound

    Slide 12 - Ionic compound

    • Example: Iron (III) and Carbonate
    • +1
    • +2
    • +3
    • -3
    • -2
    • -1
    • NH4+
    • Ammonium
    • Ca2+
    • Calcium
    • Al3+
    • Aluminium
    • O2-
    • Oxide
    • OH-
    • Hydroxide
    • Na+
    • Sodium
    • Mg2+
    • Magnesium
    • Fe3+
    • Iron (III)
    • S2-
    • Sulphide
    • Cl-
    • Chloride
    • K+
    • Potassium
    • Cu2+
    • Copper
    • CO32-
    • Carbonate
    • NO3-
    • Nitrate
    • Ag+
    • Silver
    • Pb2+
    • Lead
    • SO42-
    • Sulphate
    • HCO3-
    • Hydrogen carbonate
    • H+
    • Hydrogen
    • Fe2+
    • Iron (II)
    • Ba2+
    • Barium
    • Zn2+
    • Zinc
  13. Ionic Compound – Give it a go

    Slide 13 - Ionic Compound – Give it a go

    • Hydrogen and Chlorine (chloride)
    • Silver and Sulphar (sulphide)
    • Lead and Nitrate
    • Copper and Hydrogen carbonate
    • +1
    • +2
    • +3
    • -3
    • -2
    • -1
    • NH4+
    • Ammonium
    • Ca2+
    • Calcium
    • Al3+
    • Aluminium
    • O2-
    • Oxide
    • OH-
    • Hydroxide
    • Na+
    • Sodium
    • Mg2+
    • Magnesium
    • Fe3+
    • Iron (III)
    • S2-
    • Sulphide
    • Cl-
    • Chloride
    • K+
    • Potassium
    • Cu2+
    • Copper
    • CO32-
    • Carbonate
    • NO3-
    • Nitrate
    • Ag+
    • Silver
    • Pb2+
    • Lead
    • SO42-
    • Sulphate
    • HCO3-
    • Hydrogen carbonate
    • H+
    • Hydrogen
    • Fe2+
    • Iron (II)
    • Ba2+
    • Barium
    • Zn2+
    • Zinc
  14. Ionic Compound – Give it a go

    Slide 14 - Ionic Compound – Give it a go

    • Hydrogen and Chlorine (chloride)
    • Silver and Sulphar (sulphide)
    • Lead and Nitrate
    • Copper and Hydrogen carbonate
    • +1
    • +2
    • +3
    • -3
    • -2
    • -1
    • NH4+
    • Ammonium
    • Ca2+
    • Calcium
    • Al3+
    • Aluminium
    • O2-
    • Oxide
    • OH-
    • Hydroxide
    • Na+
    • Sodium
    • Mg2+
    • Magnesium
    • Fe3+
    • Iron (III)
    • S2-
    • Sulphide
    • Cl-
    • Chloride
    • K+
    • Potassium
    • Cu2+
    • Copper
    • CO32-
    • Carbonate
    • NO3-
    • Nitrate
    • Ag+
    • Silver
    • Pb2+
    • Lead
    • SO42-
    • Sulphate
    • HCO3-
    • Hydrogen carbonate
    • H+
    • Hydrogen
    • Fe2+
    • Iron (II)
    • Ba2+
    • Barium
    • Zn2+
    • Zinc
  15. End

    Slide 15 - End